2. Matter
Physical State Properties Changes Energy
Solid Physical Physical Exothermic
Liquid Chemical Chemical Endothermic
Gas Intrinsic
Plasma Extrinsic
3. Matter
Composition
Pure Substance Mixture Homogeneous Heterogeneous Colloid
Element Compound Solution Suspension
Metal Acid Coarse
Non-metal Base
Metalloid Salt
5. CHEMISTRY
• The science of matter, its
properties, structure, composition and its changes
during interactions and chemical reactions.
• The branch of science that deals with the
identification of the substances of which matter is
composed; the investigation of their properties and
the ways in which they interact, combine, and
change; and the use of these processes to form
new substances
6. MATTER
• anything that occupies space, possesses
mass, offers resistance and can be felt by one or
more of our senses
• Mass is the amount of matter in an object and
volume is the amount of space occupied by an
object
8. PROPERTIES
General Properties • Shape
• Color • Electrical Conductivity
• Odor • Size
• Temperature • Mass
• Taste • Weight
• Specific Gravity Special Properties
• Density • Liquid – Viscosity, Turbidity
• Effect Of Magnet • Solid –
• Solubility Ductility, Malleability, Elast
icity
9. DEFINITIONS
Physical Properties
• Properties that can be determined without
necessarily changing the chemical composition
Chemical Properties
• Properties that cannot be determined just by
viewing or touching the substance
• Signs that chemical change has occurred:
• Odor, color, or temperature change
• Precipitate or gas formation
10. DEFINITIONS
Extrinsic Properties
• Properties that are dependent to the amount of the
substance or its mass
Intrinsic Properties
• Properties that are not dependent to the amount of
the substance and is ,therefore, unaffected by
mass.
16. ENERGY USE
• Endothermic
• From a more compact state of matter, to a less compact
state of matter. (ex: solid--->gas)
• Exothermic
• From a less compact state of matter to a more compact
state of matter(ex: liquid--->solid
17. PHYSICAL
• Physical changes are changes affecting the form of
a chemical substance, but do not change the
chemical composition of that substance.
• Physical changes are used to separate mixtures into
their component compounds, but cannot usually
be used to separate compounds into chemical
elements or simpler compounds.
18. CHEMICAL
• Chemical changes occur when a substance
combines with another to form a new substance
or, alternatively, decomposes into two or more
different substances.
• These processes are called chemical reactions
and, in general, are not reversible except by further
chemical reactions.
21. PURE SUBSTANCE
• Made up of only one kink of material
• All particles are exactly the same
• Has definite properties
• Examples
• Salt
• Iron
• Water
• Can be classified into 2 groups
• Elements
• Compounds
22. ELEMENTS
• Simplest form of matter
• Atom
• Smallest particle of an element
• Atoms of the same element are alike
• Operational Definition:
• Substances that cannot be broken down any further
23. METALS
• Most are conductors of heat and energy
• Generally have high densities
• Have a fairly high melting point
• Shiny and are lustrous
• Most are ductile and malleable
• Tends to lose their outer most electrons when
chemically combined
• Most are solid at room temperature except for
mercury (Hg) which is in its liquid form
24. METALS
• Metals that are magnetic
• Iron (Fe)
• Nickel (Ni)
• Cobalt (Co)
• Reacts with water to form their metal oxide
• Operational Definition:
• Usually become basic when heated
25. NON-METALS
• Dull in appearance
• Brittle
• Don’t conduct heat and electricity
• Usually lower densities and melting points
• Tends to gain electrons when chemically combined
• Half of non-metals are gases at room
temperature, such as noble gases, except for bromine
which is liquid
• Operational Definition:
• Usually become acidic when heated
26. METALLOIDS
• Has physical properties close to metals
• Intermediate electrical conductivity
• Intermediate reflectance
• Has chemical properties close to non-metals
• Low densities and melting points
• Brittle
• Examples :
• Boron
• Silicon
• Germanium
• Arsenic
• Antimony
• Tellurium
27. COMPOUNDS
• Substances composed of 2 or more elements that
are chemically combined
• Molecule
• Smallest particle of a compound
• Operational Definition:
• Substances that can be broken down into simpler elements
(through heat/electricity
28. ACIDS
• Tastes sour
• Contains hydrogen
• Ionizes to produce positive hydrogen ions(H+) which
is a proton
• Hydrogen ions makes acids good electrolytes
• Electrolyte
• Proton donors
29. BASES
• Taste bitter
• Slippery to the touch
• Can be poisonous and corrosive
• Contains Hydroxide ions (OH-)
• Proton Acceptors
30. INDICATORS
Indicators
• Compounds that show a definite color when mixed wit an
acid or base
Substance Blue LP Red LP Methyl Orange Phenolphthalein
Acid Red Red Red Clear
Base Blue Blue Orange Magenta
31. SALT
• Formed when an acid reacts chemically with a
base. This process is called neutralization
• Neutralization is only compete when the hydrogen
and hydroxide ions are equal
HCL NaOH H2O
(Acid) (Base) NaCl
32. ELECTROLYSIS
• A chemical separation of a compound into
elements
• Anode +
• Cathode –
• Reduction
• An electron is gained
• Happens at the cathode
• Oxidation
• An electron is lost
• Happens at the anode
33. MIXTURES
• May change physical appearance when dissolved
• Operational Definition:
• A mix of matter that can be separated through physical
means
34. HETEROGENEOUS
• A mixture that does not appear to be the same
throughout
• Particles are large enough to be seen and to
separate from the mixture
• Tends to settle when the mixture is left undisturbed
• Types
• Coarse - Mostly Solid
• Suspension – Contains a liquid in which visible particles settle
• Effect of Light
• Light slightly passes through
36. SOLUTION
• The “best mixed” of all
• Particles are too small to be seen
• Formed when one substance dissolves another
• Effect of Light
• Light passes through
37. COLLOID
• Particles are not dissolved but are dispersed
• Do not settle but remain suspended for some time,
• Somewhat large particles relative to a solution
• Brownian Movement
• Effect of light
• Makes the colloid appear to glow
• The colloid scatters the light
38. SEPARATING MIXTURES
• Magnetism
• Uses magnets to separate metallic and non-metallic
components of a mixture
• Decantation
• Allowing solid particles to settle first then pouring the liquid
into another container
• Filtration
• Separating undissoved solid particles from the liquid by
allowing the liquid to pass through a filter
39. SEPARATING MIXTURES
• Evaporation
• Separating a liquid from a solid wherein the liquid part is lost
and only the solid part is recovered
• Distillation
• separating a mixture of 2 liquids by evaporating the one
with the lower boiling point
• Chromatography
• Method of physical separation making use of the adsorbent
property of a substance
41. EXPT. #3
Sample No. Physical Color Odor Solubility in Water Effect of Magnet
State
Copper Strips Solid Copper Brown Odorless Insoluble Non Magnetic
Sulfur Powder Solid Bright Yellow Reeking Insoluble Non Magnetic
Sucrose Solid Crystal White Aromatic Soluble Non Magnetic
Iodine Crystals Solid Metallic Gray Musty Slightly Soluble Non Magnetic
Ethyl Alcohol Liquid Clear Fragrant Miscible Non Magnetic
Sodium Chloride Solid Crystal White Odorless Soluble Non Magnetic
Naphthalene Solid White Fresh Insoluble Non Magnetic
Sodium Bicarbonate Solid White Odorless Slightly Soluble Non Magnetic
Copper Sulfate Solid Light Blue Odorless Slightly Soluble Non Magnetic
Dilute Acetic Acid Liquid Foggy White Pungent Miscible Non Magnetic
Acetone Liquid Clear Noxious Miscible Non Magnetic
Iron Solid Silvery Odorless Insoluble Magnetic
42. EXPT. #4
Diff. Bet. Initial and Final
Chemical System Initial State Final State
State
Lead Nitrite Colorless, Colder, Colorless, Odor and Temperature
+ Hydrochloric Acid Pungent Odorless Change
Sodium Bicarbonate Colorless, Gas Formation, Gas Formation
+ Hydrochloric Acid Odorless Colorless, Odorless
Copper Sulfate Blue, Blue, Odor Change
+ Hydrochloric Acid Metallic Smell Reeking
Potassium Chromate Yellow, Orange, Color Change
+ Hydrochloric Acid Fresh Smell Odorless
Magnesium Chloride Colorless, White, Gas Formation, Gas Formation,
+ Hydrochloric Acid Odorless Musty Odor Change
Lead Nitrite Colorless, White, Precipitate Formation
+ Ammonia Pungent Foggy, Pungent
Sodium Bicarbonate Colorless, Colder, Colorless, Odor and Temperature
+ Ammonia Odorless Pungent Change
44. EXPT. #5
Chemical System Observation Analysis
Copper turnings and sulfur The burning sulfur evaporated and left
Examined w/ lens - Copper and sulfur are separate. a noxious smell while the copper simply
- Sulfur is yellow w/ large granules. melted.
- Some of the copper is bent.
- Produced a noxious smell
- Sulfur evaporated
- Copper melted
Heated together - Copper turned black
Magnesium ribbon The magnesium ribbon heated up until
Burned in air - Yellow-green flame its flash point and burned in a bright
yellow green flame. The solution
Combustion product - Black, fragile, breaking, ashes produced a sour smell.
- Cloudy water
Dissolved in water - Grayish color
- Red turned to blue
Solution tested w/ red and blue litmus paper - Basic solution
45. Sulfur powder The sulfur powder was acidic after it was
Burned in air Turned black burned and dissolved in water
Combustion product Black, ashes
Dissolved in water Cloudy water
Solution tested w/ red and blue litmus paper Blue turned to red
Acidic solution
Iodine crystals The iodine crystals vaporized into pink
Heated Pink gas gas then formed crystals on the
Evaporation of crystals evaporating dish above. The resulting
crystals stain a yellow-orange tinge on
Shiny, gray, yellow-orange stain, no hands
Vapor cooled smell
Copper Sulfate The copper sulfate turned to white
Heated Evaporation of copper sulfate crystals indicating a chemical change
turned to white
Sodium Chloride and sand When the sand and salt was mixed, they
Examine w/ lens Sand sticks to salt can be clearly distinguished from each
other.
Mixed w/ water Cloudy brown water When mixed with water, the salt
Salt dissolved dissolved while the sand settled at the
Sand settled at the bottom bottom.
We filtered the solution and after
Murky, yellowish liquid evaporating the filtrate, the sand
Filtered Small sand particles remained.
Yellowish salt crystals
Filtrate allowed to evaporate Dark yellow middle
46. EXPT. #7
Color Odor Taste
Water Colorless Odorless Tasteless
Fresh but Sweet with a stinging
Ethyl Alcohol Colorless
Stingy aftertaste
Fresh but Sweet with a mild
1st Distillate Colorless
Stingy stinging aftertaste
Sweet with a
2nd Distillate Colorless Very Stingy dominant stinging
aftertaste
Cloudy Noxious and A mild stinging
Residue
Yellow Reeking aftertaste
47. EXPT. 8
Anode Gas Cathode Gas
Relative Volume Half compared to Two times larger in
cathode gas volume
Reaction to Fire Brightens the flame of Catches fire in a loud
the match popping noise
48. EXPT. #9
Color Ds Df Rf
Green
~ Yellow 9.9 cm. 0.9
~ Blue 10.9 cm. 0.99
~ Water 11 cm.
Blue
~ Blue 10.4 cm. 0.99
~ Water 10.5 cm.
Yellow
~ Yellow 10.3 cm. 0.9
~ Pink 9.3 cm. 0.8
~ Water 11.5 cm.
Black
~ Black 11.2 cm. 1
~ Water 11.2 cm.
